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Chapter 9: Problem 29

The \(\mathrm{Na}^{+}\) ion and the Ne atom are isoelectronic. The ease of loss of an electron by a gaseous Ne atom, \(I_{1}\) has a value of \(2081 \mathrm{kJ} / \mathrm{mol} .\) The ease of loss of an electron from a gaseous \(\mathrm{Na}^{+}\) ion, \(I_{2}\), has a value of \(4562 \mathrm{kJ} / \mathrm{mol} .\) Why are these values not the same?

Short Answer

Expert verified
The difference in Ionization energy between Na+ and Ne, even though they are isoelectronic, arises due to the difference in nuclear charge they have. Sodium Ion Na+ has a higher nuclear charge than Neon, so it has a stronger hold on its electrons. Additionally, removing an electron from Na+ would mean losing an electron from a lower energy level which is closer to the nucleus, thus needs more energy.

Step by step solution

01

Understand the Properties of Neon and Sodium Ion

Both Ne and Na+ have the same number of electrons, which is 10. Therefore, they are isoelectronic. However, they are not the same atom and they don't have the same number of protons in their nucleus which affects the ionization energy.
02

Understand Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. The ionization energy depends on the attraction between the electrons and the nucleus. If an atom has a larger nuclear charge, the electrons will be more attracted to the nucleus, requiring more energy to be removed. That's why \(I_{1}\) for Ne is 2081 kJ/mol and \(I_{2}\) for Na+ is 4562 kJ/mol.
03

Compare the Ionization Energies of Neon and Sodium Ion

Neon atom has a nuclear charge of +10 (since it has 10 protons), while sodium ion Na+ also has a nuclear charge of +11 (since it has 11 protons). The additional proton in sodium ion leads to a greater attractive force on the electrons. That's why the ionization energy of sodium ion is higher than that of Neon.
04

Understand the Difference in Ionization Energies

When we're removing the first electron from Neutral Neon, that electron is being removed from a shell that is already stable (complete shell). However, for sodium ion Na+, when the second electron is being removed, it's being removed from a lower energy level which is closer to the nucleus and hence under a much greater attractive force. This is why it takes more energy to remove an electron from Na+ than it does from Ne.

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